QuestionJune 19, 2025

How many molecules are there in 75 grams of aluminum triflouride? 5.68times 10^23 5.38times 10^23 5.98times 10^23 6.23times 10^23

How many molecules are there in 75 grams of aluminum triflouride? 5.68times 10^23 5.38times 10^23 5.98times 10^23 6.23times 10^23
How many molecules are there in 75 grams of aluminum triflouride? 5.68times 10^23 5.38times 10^23 5.98times 10^23 6.23times 10^23

Solution
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Answer

5.38 \times 10^{23} Explanation 1. Calculate Molar Mass of Aluminum Trifluoride The molar mass of AlF_3 is calculated as follows: Al = 26.98 \, g/mol, F = 18.998 \, g/mol. Therefore, AlF_3 = 26.98 + 3 \times 18.998 = 83.976 \, g/mol. 2. Calculate Moles of Aluminum Trifluoride Use the formula: **moles = \frac{mass}{molar \, mass}**. For 75 \, g of AlF_3: \frac{75}{83.976} \approx 0.893 \, moles. 3. Calculate Number of Molecules Use Avogadro's number: **number \, of \, molecules = moles \times 6.022 \times 10^{23}**. Thus, 0.893 \times 6.022 \times 10^{23} \approx 5.38 \times 10^{23} molecules.

Explanation

1. Calculate Molar Mass of Aluminum Trifluoride<br /> The molar mass of $AlF_3$ is calculated as follows: $Al = 26.98 \, g/mol$, $F = 18.998 \, g/mol$. Therefore, $AlF_3 = 26.98 + 3 \times 18.998 = 83.976 \, g/mol$.<br />2. Calculate Moles of Aluminum Trifluoride<br /> Use the formula: **moles = \frac{mass}{molar \, mass}**. For $75 \, g$ of $AlF_3$: $\frac{75}{83.976} \approx 0.893 \, moles$.<br />3. Calculate Number of Molecules<br /> Use Avogadro's number: **number \, of \, molecules = moles \times 6.022 \times 10^{23}**. Thus, $0.893 \times 6.022 \times 10^{23} \approx 5.38 \times 10^{23}$ molecules.
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